Answered: Write the complete chemical equation of…

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Write the complete chemical equation of leaching Cuo in acidic solution which produces Cu²* ions. www

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter20: Chemistry Of Hydrogen, Elements In Group 3a Through 6a, And The Noble Gases

Section: Chapter Questions

Problem 20.46QE

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Using data in Appendix 1, estimate the temperature at which Fe2O3 can be reduced to iron, using hydrogen gas as a reducing agent (assume H2O(g) is the other product).
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An ore containing magnetite, Fe3O4 was analyzed by dissolving a 1.5419 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
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An ore containing magnetite, Fe3O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCl, giving a mixture of Fe2+ and Fe³+. After adding HNO3 to oxidize any Fe²+ to Fe³+, the resulting solution was diluted with water and the Fe³+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe₂O3. Calculate the %w/w Fe3O4 in the sample.